🤓 Based on our data, we think this question is relevant for Professor Hilty's class at TAMU.

In 1897 the Swedish explorer Andreé tried to reach the North Pole in a balloon. The balloon was filled with hydrogen gas. The hydrogen gas was prepared from iron splints and diluted sulfuric acid. The reaction is

Fe(*s*) + H_{2}SO_{4}(*aq*) → FeSO_{4}(*aq*) + H_{2}(*g*)

The volume of the balloon was 4800 m^{3} and the loss of hydrogen gas during filling was estimated at 20.%. What mass of iron splints and 98% (by mass) H_{2}SO_{4} were needed to ensure the complete filling of the balloon? Assume a temperature of 0°C, a pressure of 1.0 atm during filling, and 100% yield.

- First need find
**how much moles of H**does a_{2}**4800 m**^{3}balloon contain. - We will be using the
**ideal gas equation**to**find the moles of H**using the conditions provided_{2} - The
**moles of H**_{2}is**related to the moles of Fe and H**_{2}SO_{4 }**using the balanced equation**provided which in turn will**give**us the**mass Fe and H**_{2}SO_{4 } - For the
**volume of H**_{2}, if there was 20% loss, this means that**4800 m**is^{3}**80%****of the****total H**_{2}that was produced (assuming that 20% is in volume as well)